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Intermolecular Forces and Liquids and Solids. Chapter 11. A phase is a homogeneous part of the system in contact with other parts of the system but separated from them by a well-defined boundary. 2 Phases. Solid phase - ice. Liquid phase - water. 11.1. - PowerPoint PPT Presentation
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A phase is a homogeneous part of the system in contact with other parts of the system but separated from them by a well-defined boundary.
2 Phases
Solid phase - ice
Liquid phase - water
11.1
Intermolecular Forces
11.2
Intermolecular forces are attractive forces between molecules.
Intramolecular forces hold atoms together in a molecule.
Intermolecular vs Intramolecular
• 41 kJ to vaporize 1 mole of water (inter)
• 930 kJ to break all O-H bonds in 1 mole of water (intra)
Generally, intermolecular forces are much weaker than intramolecular forces.
“Measure” of intermolecular force
boiling point
melting point
Hvap
Hfus
Hsub
Types of Intermolecular Forces1. Hydrogen Bond (strongest)
11.2
The hydrogen bond is a special dipole-dipole interaction between the hydrogen atom in a polar N-H, O-H, or F-H bond and an electronegative O, N, or F atom. IT IS NOT A BOND.
A H…B A H…Aor
A & B are N, O, or F
Why is the hydrogen bond considered a “special” dipole-dipole interaction?
Decreasing molar massDecreasing boiling point
11.2
Types of Intermolecular Forces
2. Ion-Dipole Forces
Attractive forces between an ion and a polar molecule
11.2
Ion-Dipole Interaction
Types of Intermolecular Forces
3. Dipole-Dipole Forces
Attractive forces between polar molecules
Orientation of Polar Molecules in a Solid
11.2
Types of Intermolecular Forces4. Dispersion Forces – van der Walls forces/London forces (weakest)
Attractive forces that arise as a result of temporary dipoles induced in atoms or molecules
11.2
ion-induced dipole interaction
dipole-induced dipole interaction
Intermolecular Forces4. Dispersion Forces Continued
11.2
Polarizability is the ease with which the electron distribution in the atom or molecule can be distorted.
Polarizability increases with:
• greater number of electrons
• more diffuse electron cloud
Dispersion forces usually increase with molar mass.
SO
O
What type(s) of intermolecular forces exist between each of the following molecules?
HBrHBr is a polar molecule: dipole-dipole forces. There are also dispersion forces between HBr molecules.
CH4
CH4 is nonpolar: dispersion forces.
SO2
SO2 is a polar molecule: dipole-dipole forces. There are also dispersion forces between SO2 molecules.
11.2
Properties of Liquids
Surface tension is the amount of energy required to stretch or increase the surface of a liquid by a unit area.
Strong intermolecular
forces
High surface tension
11.3
Properties of Liquids
Cohesion is the intermolecular attraction between like molecules
11.3
Adhesion is an attraction between unlike molecules
Adhesion
Cohesion
attracted to glass
attracted to each other
Properties of Liquids
Viscosity is a measure of a fluid’s resistance to flow.
11.3
Strong intermolecular
forces
High viscosity
A crystalline solid possesses rigid and long-range order. In a crystalline solid, atoms, molecules or ions occupy specific (predictable) positions.
An amorphous solid does not possess a well-defined arrangement and long-range molecular order.
A unit cell is the basic repeating structural unit of a crystalline solid.
Unit Cell
latticepoint
Unit cells in 3 dimensions 11.4
At lattice points:
• Atoms
• Molecules
• Ions
Types of Crystals
Ionic Crystals – Ion-Ion interactions are the strongest (including the “intermolecular forces” (H bonding, etc.)
• Lattice points occupied by cations and anions• Held together by electrostatic attraction• Hard, brittle, high melting point• Poor conductor of heat and electricity
CsCl ZnS CaF2
11.6
Types of Crystals
Covalent Crystals – Stronger than IM forces but generally weaker than ion-ion
• Lattice points occupied by atoms• Held together by covalent bonds• Hard, high melting point• Poor conductor of heat and electricity
11.6diamond graphite
carbonatoms
Types of Crystals
Molecular Crystals• Lattice points occupied by molecules• Held together by intermolecular forces• Soft, low melting point• Poor conductor of heat and electricity
11.6
Types of Crystals
Metallic Crystals – Typically weaker than covalent, but can be in the low end of covalent
• Lattice points occupied by metal atoms• Held together by metallic bonds• Soft to hard, low to high melting point• Good conductors of heat and electricity
11.6
Cross Section of a Metallic Crystal
nucleus &inner shell e-
mobile “sea”of e-
An amorphous solid does not possess a well-defined arrangement and long-range molecular order.
A glass is an optically transparent fusion product of inorganic materials that has cooled to a rigid state without crystallizing
Crystallinequartz (SiO2)
Non-crystallinequartz glass 11.7
The equilibrium vapor pressure is the vapor pressure measured when a dynamic equilibrium exists between condensation and evaporation
H2O (l) H2O (g)
Rate ofcondensation
Rate ofevaporation=
Dynamic Equilibrium
11.8
Molar heat of vaporization (Hvap) is the energy required to vaporize 1 mole of a liquid.
ln P = -Hvap
RT+ C
Clausius-Clapeyron EquationP = (equilibrium) vapor pressure
T = temperature (K)
R = gas constant (8.314 J/K•mol)
11.8
C = constant (depends on P & T)
The boiling point is the temperature at which the (equilibrium) vapor pressure of a liquid is equal to the external pressure.
The normal boiling point is the temperature at which a liquid boils when the external pressure is 1 atm.
11.8
The critical temperature (Tc) is the temperature above which the gas cannot be made to liquefy, no matter how great the applied pressure.
The critical pressure (Pc) is the minimum pressure that must be applied to bring about liquefaction at the critical temperature.
11.8
Mel
ting
11.8F
reez
ing
H2O (s) H2O (l)
The melting point of a solid or the freezing point of a liquid is the temperature at which the solid and liquid phases coexist in equilibrium
Sub
limat
ion
11.8
Dep
ositi
on
H2O (s) H2O (g)
Molar heat of sublimation (Hsub) is the energy required to sublime 1 mole of a solid.
Hsub = Hfus + Hvap
( Hess’s Law)
A phase diagram summarizes the conditions at which a substance exists as a solid, liquid, or gas.
The triple point is where all 3 phases meet.
Phase Diagram of Water
11.9
Where’s Waldo?Can you find…
The Triple Point?
Critical pressure?
Critical temperature?
Where fusion occurs?
Where vaporization occurs?
Melting point (at 1 atm)?
Boiling point(at 6 atm)?
Carbon Dioxide
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